An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C Cl₂(g) + 2 e 2 Cl-(aq) 1.360 O₂(g) + 4 H30+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(l) + 2 e² →→→ H₂(g) + 2 OH-(aq) -0.828 Cd²+ (aq) + 2 e² → Cd(s) -0.403 + + (b) What is the expected decomposition potential? + + + +
An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C Cl₂(g) + 2 e 2 Cl-(aq) 1.360 O₂(g) + 4 H30+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(l) + 2 e² →→→ H₂(g) + 2 OH-(aq) -0.828 Cd²+ (aq) + 2 e² → Cd(s) -0.403 + + (b) What is the expected decomposition potential? + + + +
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.50QE
Related questions
Question
![Half-reaction at anode:
Use the References to access important values if needed for this question.
An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes.
(a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below.
Standard Reduction Potentials (Volts) at 25 °C
2 Cl-(aq)
1.360
Cl₂(g) + 2 e-
O₂(g) + 4 H3O+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229
2 H₂O(1) + 2 e¯ →→ H₂(g) + 2 OH-(aq)
Cd²+(aq) + 2 e² →→ Cd(s)
-0.828
-0.403
Half-reaction at cathode:
Enter electrons as e.
Use smallest possible integer coefficients.
States are not required. If a box is not needed, leave it blank.
+
(b) What is the expected decomposition potential?
V
+
+
+
+](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd295e1c3-483d-49b7-8dbf-fcde864060f6%2F8d7e3a45-e460-4d5a-b8f5-6e687caad2a9%2Fz0wfeqp_processed.png&w=3840&q=75)
Transcribed Image Text:Half-reaction at anode:
Use the References to access important values if needed for this question.
An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes.
(a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below.
Standard Reduction Potentials (Volts) at 25 °C
2 Cl-(aq)
1.360
Cl₂(g) + 2 e-
O₂(g) + 4 H3O+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229
2 H₂O(1) + 2 e¯ →→ H₂(g) + 2 OH-(aq)
Cd²+(aq) + 2 e² →→ Cd(s)
-0.828
-0.403
Half-reaction at cathode:
Enter electrons as e.
Use smallest possible integer coefficients.
States are not required. If a box is not needed, leave it blank.
+
(b) What is the expected decomposition potential?
V
+
+
+
+
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 4 steps with 10 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry: Principles and Practice](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
![Chemistry & Chemical Reactivity](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning